Alkalinity is determined by several factors such as rocks, soil, salts and certain industrial activities waste water containing soap and detergents are alkaline by man.
For example, the areas where limestone CaCO 3 is significantly available can have more alkaline water. Basicity: Factors affecting the basicity of a compound vary depending on the definition of the basicity. For example, electron pair availability of a base depends on three factors.
When considering the atoms in the same row in the periodic table, the most electronegative atom has the higher basicity. When considering a row of the periodic table, the larger the atom has the less electron density and it is less basic. Molecules having more resonance structures are less basic, since the less electron availability than a localized negative charge.
Coming from Engineering cum Human Resource Development background, has over 10 years experience in content developmet and management. Your email address will not be published. Leave a Reply Cancel reply Your email address will not be published. Originally Posted by jrivanov. To further expound on Doc Roddy's answer he's the chemist I'm a wannabe Adding more of the drops adds more acid to the sample and more coloring too.
Eventually the pH "crashes" in the sample as all of the carbonate buffers are depleted. At this point the color of the test sample changes indicating the end of the test. The side effect of this type of test is you can scale the results up or down depending on the resolution you need. Since each drop is now indicative of Conversely, if you're trying to do accurate testing and cant afford "lab-grade" tests, you can double the size of the test sample.
Now each "drop" of titrant isn't In theory, you can scale things either direction by an order of magnitude if you wanted to do so, but mostly folks stick with the baseline of a 5 mL sample and Make sense? Thanks you guys that does make sense.
Great idea especially when I am trying to keep the KH above ppm bead filter it also makes for a much quicker test. Off subject a little but by raising Kh am I affecting the hardness of the water?
Or is that only by raising the GH? By raising the level to ppm for example, is the water harder or softer than it was at a 58 ppm level? I have read on the board that harder water brings some colors out more and supresses some more, is this also true? Thanks all in advance. Mechanic by trade. Others may disagree.
I can show you examples of such changes happening both ways, but they're not uniform, across-the-board truths. So YMMV. The same is not necessarily true in domestic fish. Example: Sometimes I can take a Rowley fish which looks really good in hard water, and watch it get somewhat mushy in very soft water. Other times, they look better, while other times they don't give a flip what you've got for water as long as you're not beating them on the head with a rock.
If I had to guess, I'd say that "fish do the best in waters which replicate the parameters found in their ancestral homes". Sorta makes sense if you think about it. As to making the water "harder" by adding bicarb etc , the answer to that question is "Yes and No", for reasons having to do with the definition of "hardness".
In nature, ionic compounds salts contain alkali metals but never in a pure state. Alkaline bases include a slimy or soapy feel to the touch because of saponification of fatty acids in human skin. Alkalis form hydroxide ions OH- when dissolved in water and all are Arrhenius bases.
Normally water-soluble, some alkalis, such as barium carbonate, become soluble only when reacting with an acidic solution containing water. Moderately concentrated solutions pH of 7. Concentrated solutions cause chemical burns caustic. Named for Johannes Bronsted and Thomas Lowry, a Brosted-Lowry base is any substance that accepts a hydrogen icon proton.
A BL acid is any substance that rejects a hydrogen ion, as stated on the New York University website. The Arrhenius definition, on the other hand, classifies a base as any substance that increases the concentration of hydroxide ions in water OH-.
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